+18-01 Q3. Calculate the [H] (concentration of the H*) of a HCI solution when the pH=2.88 **Hint to solve Q3: antilog pH = -log[H] Molar mass HC1= 36.458 CH*]=9+iles (PH) 10-288 ↓ 1.318x10 n mol 13x10-3 ml g mol Density HCI-1.18 ml
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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![**Question 3:**
Calculate the [H⁺] (concentration of H⁺) of an HCl solution when the pH = 2.88.
**Hint to solve Q3: antilog**
\[ \text{pH} = -\log[\text{H}^+] \]
\[ \text{Molar mass HCl} = 36.458 \, \text{g/mol} \]
\[ \text{Molar mass H₃PO₄} = 97.994 \, \text{g/mol} \]
\[ \text{Density HCl} = 1.18 \, \text{g/ml} \]
\[ \text{Density H₃PO₄} = 1.88 \, \text{g/ml} \]
**Solution steps (handwritten):**
- \( [\text{H}^+] = 10^{-\text{pH}} = 10^{-2.88} \)
- \( 1.318 \times 10^{-3} \, \text{M} \)
- \(\approx 1.3 \times 10^{-3} \, \text{M} \)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F21c9e2c1-3922-4190-983a-755fc6e01f0b%2F6aecb197-dd6a-4f82-a8ef-8da22f548f69%2F4ka028_processed.jpeg&w=3840&q=75)
pH of the HCl solution = 2.88
Concentration of the H+ ion = [H+] = ?
Note: As we know that,
pH = -log[H+]
[H+] = 10-pH
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